The average atomic mass of a hypothetical element is 139.85 amu. Determine the missing abundances of...
Part A What is the relative atomic mass of a hypothetical element that consists of the following isotopes in the indicated natural abundances? Isotope Isotopic mass (amu) Relative abundance (%) 1 81.9 12.2 2 84.9 15.0 3 88.9 72.8 Express your answer to three significant figures and include the appropriate units. Part B What is the relative atomic mass of the element that consists of the following isotopes in the indicated natural abundances? Isotope Isotopic mass (amu) Relative abundance (%)...
5. An element consists of two isotopes in the indicated natural abundances: Isotope A, mass=84.9118 amu, abundance = 72.15% Isotope B, mass = 86.9092 amu, abundance = 27.85% What is the atomic weight of this element? What is the identity of the element? Show your calculations.
Part A What is the relative atomic mass of a hypothetical element that consists of the following isotopes in the indicated natural abundances? Isotope Isotopic mass Relative abundance (amu) (%) 78.9 82.9 13.0 120 869 750 Express your answer to three significant figures and include the appropriate units.
The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is _ _amu. Isotope Abundance (%) Mass (amu) 221X 74.22 220.90 12.78 220.00 2187 13.00 218.10 2207 219.70 220.34 220.43 219.00 33.333
The hypothetical element Q has an atomic weight of 124.8 AMU in the periodic table and only has two stable isotopes. Q isotope 1 has an abundance of 55.83 % and an isotopic mass of 122.16 AMU. What is the mass of Q isotope in AMU ? Round 3 decimal places.
An element has three naturally occurring isotopes with masses as listed below. The average atomic mass of this element is 28.08 amu. Determine the two missing percent abundances.^28X 27.98 amu % abundance =^29X 28.98 amu % abundance = 4.68 %^30X 29.97 amu % abundance =
On another planet, the isotopes of titanium have the given natural abundances. Isotope Abundance Mass (amu) 46Ti 77.100% 45.95263 48Ti 11.700% 47.94795 50Ti 11.200% 49.94479 What is the average atomic mass of titanium on that planet? _______=amu
The element carbon has two naturally occurring isotopes. The isotopic masses and abundances of these isotopes are shown in the table below. Isotope 12c isotopic mass (amu) Abundance (%) 12.00 13.00 98.93 1.07 Calculate the average atomic mass of carbon to two digits after the decimal point. Number = _______ amu
QUESTION 3 A fictitious element is composed of isotopes A and B with masses of 61.9887 and 64.9846 amu respectively. The average atomic mass of the element is 64.52 amu. What can you conclude about the natural abundances of the two isotopes? O The natural abundance of isotope A must be greater than that of isotope B OThe natural abundance of isotope B must be greater than that of isotope A. O The natural abundances of both isotopes must be...
Most elements occur naturally as a mix of different isotopes. An element's atomic mass is the weighted average of the isotope masses. In other words, it is an average that takes into account the percentage of each isotope. For example, the two naturally occurring isotopes of boron are given here The atomic mass of boron is calculated as follows: (10.0 times 0.199) + (11.0 times 0.801) = 10.8 amu Because the heavier isotope is more abundant the atomic mass a...